The Condensed Phases: Liquids and Solids

Learning Objectives

Following your study of this chapter, you should be able to

1. use a kinetic-molecular model to describe the structure of a liquid and a solid;

2. characterize the enthalpy associated with any phase change;

3. plot the cooling or heating curve for a pure substance;

4. calculate the enthalpy changes along a cooling or heating curve given the specific heat for each phase and the enthalpy for each phase change;

5. define the term equilibrium vapor pressure and sketch the kinetic-molecular model of a liquid in equilibrium with its vapor;

6. determine the experimental vapor pressure for a liquid using a barometer;

7. describe how temperature effects the vapor pressure of a liquid using kinetic-molecular model;

8. write and use the mathematical equation that describes the dependence of vapor pressure on temperature;

9. define the terms, boiling point, viscosity and surface tension;

10. define and illustrate using diagrams of atoms, ions or molecules, the inter-molecular attractive forces: ion-dipole, dipole-dipole, London dispersion and hydrogen-bonding;

11. predict the major types of intermolecular attractive force that occur between any two particles in the liquid phase;

12. distinguish between crystalline solids and amorphous solids;

13. identify and give representative examples of atomic solids, molecular solids, ionic solids, covalent solids, and metals;

14. illustrate the characteristic packing arrangement for simple cubic, body-centered cubic and face-centered cubic lattices;

15. define the term unit cell and draw the unit cell for simple cubic, body-centered cubic and face-centered cubic lattices;

16. determine the number of particles in a unit cell for simple cubic, body-centered cubic and face-centered cubic lattices;

17. distinguish between hexagonal and cubic closest-packing;

18. identify crystal defects and describe their effects on the properties of solids;

19. draw the phase diagram for a pure substance and label the axis and all important features;

20. describe the physical changes in a pure substance when the temperature is changed at constant pressure or when the pressure is changed at constant temperature.

 

This is a set of learning objectives from an AP Chemistry course taught via satellite by John Gelder in the early 1990's.